State the law of thermodynamics that was first formulated by Nernst in 1906. What is the utility of this law? The equilibrium constant for the reaction A ⇌ B is 1 . 8 × 10 - 7 at 298 K . Calculate the value of ∆ G º for the reaction ( R = 8 . 314 J K - 1 mol - 1 ) . Predict the feasibility of the reaction under standard states.

The third law of thermodynamics states that the entropy of a perfect crystal at a temperature of zero Kelvin (absolute zero) is equal to zero. The third law is based on the postulate of Nernst to explain empirical rules for equilibrium of chemical reactions as absolute zero is approached. As a consequence of the third law, the following quantities vanish at absolute zero: heat capacity, coefficient of thermal expansion, and ratio of thermal expansion to isothermal compressibility. The equilibrium constant for the reaction A ⇌ B is 1 . 8 × 10 - 7 at 298 K . Relationship Standard Free Energy Change and Equilibrium Constant, ΔG ° = − 2 . 303 RTlogK ΔG ° = - 2 . 303 × 8 . 314 J K - 1 mol - 1 × 298 K × log 1 . 8 × 10 - 7 ΔG ° = 38484 . 39 J ΔG ° is positive, hence the reaction isn't feasible.

State the law of thermodynamics that was first formulated by Nernst in 1906. What is the utility of this law? The equilibrium constant for the reaction A ⇌ B is 1 . 8 × 10 - 7 at 298 K . Calculate the value of ∆ G º for the reaction ( R = 8 . 314 J K - 1 mol - 1 ) . Predict the feasibility of the reaction under standard states.

The third law of thermodynamics states that the entropy of a perfect crystal at a temperature of zero Kelvin (absolute zero) is equal to zero. The third law is based on the postulate of Nernst to explain empirical rules for equilibrium of chemical reactions as absolute zero is approached. As a consequence of the third law, the following quantities vanish at absolute zero: heat capacity, coefficient of thermal expansion, and ratio of thermal expansion to isothermal compressibility. The equilibrium constant for the reaction A ⇌ B is 1 . 8 × 10 - 7 at 298 K . Relationship Standard Free Energy Change and Equilibrium Constant, ΔG ° = − 2 . 303 RTlogK ΔG ° = - 2 . 303 × 8 . 314 J K - 1 mol - 1 × 298 K × log 1 . 8 × 10 - 7 ΔG ° = 38484 . 39 J ΔG ° is positive, hence the reaction isn't feasible.

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11th ICSE

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State the law of thermodynamics that was first formulated by Nernst in 1906. What is the utility of this law? The equilibrium constant for the reaction $A ⇌ B$ is $1.8 \times 10^{- 7}$ at $298 K$ . Calculate the value of $∆ G º$ for the reaction $(R = 8.314 J K^{- 1} {mol}^{- 1})$ . Predict the feasibility of the reaction under standard states.

Important Questions on Thermodynamics

EASY

11th ICSE

IMPORTANT

ALL IN ONE ISC Chemistry CLASS 11>Chapter 6 - Thermodynamics>Chapter Practice>Q 23

Two moles of a perfect gas undergo the following processes :

(i) a reversible isobaric expansion from $(1.0 atm, 20.0 L)$ to $(1.0 atm, 40.0 L)$

(ii) a reversible isochoric change of state from $(1.0 atm, 40.0 L)$ to $(0.5 atm, 40.0 L)$

(iii) a reversible isothermal compression from $(0.5 atm, 40.0 L)$ to $(1.0 atm, 20.0 L)$

Sketch with labels each of the processes on the same $p - V$ diagram.

MEDIUM

11th ICSE

IMPORTANT

ALL IN ONE ISC Chemistry CLASS 11>Chapter 6 - Thermodynamics>Chapter Practice>Q 23

Two moles of a perfect gas undergo the following processes :

(i) a reversible isobaric expansion from $(1.0 atm, 20.0 L)$ to $(1.0 atm, 40.0 L)$

(ii) a reversible isochoric change of state from $(1.0 atm, 40.0 L)$ to $(0.5 atm, 40.0 L)$

(iii) a reversible isothermal compression from $(0.5 atm, 40.0 L)$ to $(1.0 atm, 20.0 L)$

Calculate the total work $(W)$ and the total heat change $(q)$ involved in the above processes.

EASY

11th ICSE

IMPORTANT

ALL IN ONE ISC Chemistry CLASS 11>Chapter 6 - Thermodynamics>Chapter Practice>Q 23

Two moles of a perfect gas undergo the following processes :

(i) a reversible isobaric expansion from $(1.0 atm, 20.0 L)$ to $(1.0 atm, 40.0 L)$

(ii) a reversible isochoric change of state from $(1.0 atm, 40.0 L)$ to $(0.5 atm, 40.0 L)$

(iii) a reversible isothermal compression from $(0.5 atm, 40.0 L)$ to $(1.0 atm, 20.0 L)$

Sketch with labels each of the processes on the same $p - V$ diagram.

MEDIUM

11th ICSE

IMPORTANT

ALL IN ONE ISC Chemistry CLASS 11>Chapter 6 - Thermodynamics>Chapter Practice>Q 23

Two moles of a perfect gas undergo the following processes :

(i) a reversible isobaric expansion from $(1.0 atm, 20.0 L)$ to $(1.0 atm, 40.0 L)$

(ii) a reversible isochoric change of state from $(1.0 atm, 40.0 L)$ to $(0.5 atm, 40.0 L)$

(iii) a reversible isothermal compression from $(0.5 atm, 40.0 L)$ to $(1.0 atm, 20.0 L)$

Sketch with labels each of the processes on the same $P - V$ diagram.

EASY

11th ICSE

IMPORTANT

ALL IN ONE ISC Chemistry CLASS 11>Chapter 6 - Thermodynamics>Chapter Practice>Q 23

Two moles of a perfect gas undergo the following processes :

(i) a reversible isobaric expansion from $(1.0 atm, 20.0 L)$ to $(1.0 atm, 40.0 L)$

(ii) a reversible isochoric change of state from $(1.0 atm, 40.0 L)$ to $(0.5 atm, 40.0 L)$

(iii) a reversible isothermal compression from $(0.5 atm, 40.0 L)$ to $(1.0 atm, 20.0 L)$

What will be the value of $∆ U, ∆ H$ and $∆ S$ for the overall process?

Important Questions on Thermodynamics

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